mdm. everything Flashcards
what determines the electric field behaviour
- direction of deflection (charge)
- angle of deflection
what is the angle of deflection changed by
- the magnitude of particle: determined by charge and mass
what are the three laws to explain electronic configurations
- Aufbom (4s>3d)
- Hund’s ( minimise inter-electronic repulsion)
- Pauli Exclusion
what did the pauli exclusion theory explain
2 electrons of opposite spins will counterbalance the electrical repulsion (from identical charges)
what affects the electrostatic effects
- number of electronic shells
- nuclear charge
- shielding effect
what does electronegativity depend on
the electrostatic forces of attraction between the nucleus and valence electrons
what does the ionic bond strength depend on
- charge (from electrostatic attraction)
- radius/size (inter-ionic dist)
what determines the strength of metallic bonds
- number of valence electrons available
- cation charges
- cation sizes
what is the bond angle affeted by
electronegativity and number of lone pair electrons
describe idid moments
momentary movements of electrons in particles will cause the electron density to be unsymmetrical: instantaneous dipole will induce a dipole on neighbouring particles, which attraction is short-lived as the electrons keep moving and the dipoles vanish and reform
what affects idid
- number of electrons/electron cloud size (size and ease of polarisability)
- surface area for molecular interaction (straight chains>branched)
what is hydrogen bonding
the highly electronegative hydrogen atom can form a particularly strong attraction with lone pair electrons on adjacent molecules and the intermolecular FOA= hydrogen bonding
what is covalent bond strength
average energy required to break one mole of a particular bond in gaseous state
what affects the covalent bond strength
- effectiveness of overlap
- number of bonds between the atom
- bond polarity
what are the effects of hydrogen bonding (IMFOA)
- explain diff in b.p of grp 4, 5, 6
- b.p of NH3 and HF
- open structure of ice
- dimerisation of carboxylic acids
carboxylic acids are dimers in
- vapour state
- non-polar solvents
what determines the degree of covalence
- cation’s polarising power
- anion’s polarising power
what affects the solubility
- strength of bond
- extensiveness of hydrogen bonding
what are the three gaseous laws
- avogradro’s law
- gay-lussac’s law ( pressure and temp)
- charles (vol. and temp)
- bolyes’ (volxpressure=vol. pa)
what is 1atm and 1 bar equivalent to
101325 Pa and 10^6 Pa
what does the kinetic theory of gases state
- particles of negligible volume
- particles of negligible attractive forces
- in constant random motion
- perfectly elastic collisions
- avg KE directly proportional to absolute temp
2 conditions real gases become more ideal
- higher temp (overcome IMF=negligible)
- lower pressure (particles’ volume become negligible compared to container’s volume)
why are gases not ideal
particles have a finite volume and size; the presence of attractive forces between gas particles
what determines the extent of positive and negative deviations
- bondings btwn (strong/weak idid/ pdpd/H bonding)
- larger electron cloud size (stronger intermolecular attractions and more easily POLARISED)
units of ideal gas equation
pV=nRT
*p=Pa
*V=m^3
*T=Kelvin
factors affecting lattice energy
- effect of ionic charge (bigger cation/anionic charge–> greater MAGNITUDE)
- effect of ionic size (smaller=larger magnitude)
assumptions made during experimental
- density of solution=density of water
- specific heat capacity refers to water’s
- heat loss to surroundings CORRECTED by extrapolation
